Free Printable Stoichiometry Intro Exit Ticket

1.

What is the first thing you must do to solve a stoichiometry problem?

a)

Write a Balanced Equation

b)

Panic

c)

Write an Unbalanced Equation

d)

Ask for help

2.

Mole Ratios used for conversions are derived from:

a)

the molar mass of the reactants in the balanced chemical equation

b)

the coefficients of the balanced chemical equation

c)

the subscripts of the products in the balanced chemical equation

d)

the group number of each element in the balanced chemical equation

3.

What are the missing coefficients for the unbalanced equation below?

Cr_(s)+ Fe(NO₃)_2(aq) → Fe_(s) + Cr(NO₃)_3(aq)

a)

2,3,3,2

b)

1,3,3,1

c)

2,3,2,3

d)

2,3,1,2

4.

When setting up a problem using mole ratios, remember to use dimensional analysis. Start with the given. The unit that the given has needs to be on bottom in the next ratio so it will cancel out. Make sure to label with both unit and chemical formula.

Using the following BALANCED chemical equation.
$4NH_3+6NO\rightarrow5N_2+6H_2O$
Bacteria will cause ammonia $NH_3$ to react with NO to put nitrogen back in the air, along with water, as part of the nitrogen cycle. If there are 3.56 moles of NO in the soil, how many moles of ammonia are needed to react with it?

$\frac{3.56\ moles\ NO}{ }\times\frac{\ \ \ \ \ ?\ \ \ \ }{?}$

a)

$\frac{\ 6\ mole\ NO}{4\ mole\ NH_3}$

b)

$\frac{2\ mole\ NH_3}{3\ mole\ NO}$

c)

$\frac{6\ mole\ Hg}{5\ mole\ N_2}$

5.

When setting up a problem using mole ratios, remember to use dimensional analysis. Start with the given. The unit that the given has needs to be on bottom in the next ratio so it will cancel out. Make sure to label with both unit and chemical formula.
Using the following BALANCED chemical equation....
$4NH_3+6NO\rightarrow5N_2+6H_2O$
How many moles of water will be produced with 3.56 moles of NO in the soil?

$\frac{3.56\ moles\ NO}{ }\times\frac{\ \ \ \ \ ?\ \ \ \ }{?}$

a)

$\frac{\ 6\ mole\ NO}{6\ mole\ H_2O}$

b)

$\frac{1\ mole\ H_2O}{1\ mole\ NO}$

c)

$\frac{6\ mole\ H_2O}{5\ mole\ N_2}$

6.

Using the reaction below,

4Al + 3O₂ → 2Al₂O₃

How many moles of aluminum oxide are produced from 6 moles of oxygen?

a)

8 mol

b)

6 mol

c)

4 mol

d)

2 mol

7.

What is the correct setup for the following problem?

How many moles are in 12.4 grams of Helium?

a)

$12.4\ g\ He\ x\ \frac{4.003g\ He}{1\ mole\ He}$

b)

$12.4\ g\ He\ x\ \frac{1\ mole\ He}{4.003\ g\ He}$

c)

$4.003\ g\ He\ x\ \frac{12.4\ g\ He}{1\ mole\ He}$

d)

$4.003\ g\ He\ x\ \frac{1\ mole\ He}{12.4\ g\ He}$

8.

When setting up a problem using mole ratios, remember to use dimensional analysis. Start with the given. The unit that the given has needs to be on bottom in the next frame so it will cancel out. Make sure to label with both unit and chemical formula.

Using the following BALANCED chemical equation....
If I decompose 34 moles of HgO, how many moles of oxygen will I produce? What will the ratio that you use look like in this problem?

$\frac{34\ moles\ HgO}{ }\times\frac{\ \ \ \ \ ?\ \ \ \ }{?}$

a)

$\frac{1mole\ O_2}{2\ mole\ HgO}$

b)

$\frac{2\ mole\ HgO}{1\ mole\ O_2}$

c)

$\frac{2\ mole\ Hg}{1\ mole\ O_2}$

9.

To convert from moles to grams, you should multiply by ....

a)

b)

c)

d)

10.

To convert from grams to moles, you should multiply by ....

a)

b)

c)

d)

11.

Baking soda is commonly used in baking to make food (such as bread) rise. The primary ingredient in baking soda is sodium bicarbonate (NaHCO₃).

What is the molar mass of this compound (NaHCO₃)?

a)

84.01 g/mol

b)

52.01 g/mol

c)

107.00 g/mol

d)

42.00 g/mol

12.

Calcium nitrate is mainly used as a fertilizer. The compound as the formula Ca(NO₃)₂ .

What is the molar mass of this compound?

a)

102.09 g/mol

b)

164.10 g/mol

c)

70.09 g/mol

d)

130.10 g/ol

13.

You want to determine the mass of 3.75 moles of Mg₃N_{2 .}

Which of the following shows the correct set-up for this calculation?

a)

b)

c)

d)

14.

You want to know how many moles O₂ are needed to react with 0.68 moles of Fe.

Which of the following shows the correct set-up for this problem?

(See image for balance equation)

a)

b)

c)

d)

15.

2 H₂ + O₂ → 2 H₂O

Which setup correctly determines the mass of H₂O produced if you begin with 50 grams of O₂?

a)

$\frac{50\ g\ O_2}{1}\times\frac{32.00\ g\ O_2}{1\ mole\ O_2}\times\frac{2\ mole\ H_2O}{1\ mole\ O_2}\times\frac{1\ mole}{18.02\ g\ H_2O}$

b)

$\frac{50\ g\ O_2}{1}\times\frac{1\ mole\ O_2}{32.00\ g\ O_2}\times\frac{2\ mole\ H_2O}{1\ mole\ O_2}\times\frac{18.02\ g\ H_2O}{1\ mole\ H_2O}$

c)

$\frac{50\ g\ O_2}{1}\times\frac{2\ mole\ H_2O}{1\ mole\ O_2}\times\frac{18.02\ g\ H_2O}{1\ mole\ H_2O}$

d)

$\frac{50\ g\ O_2}{1}\times\frac{1\ mole\ O_2}{32.00\ g\ O_2}\times\frac{18.02\ g\ H_2O}{1\ mole\ H_2O}$

Stoichiometry Intro Exit Ticket

Total questions: 15

Worksheet time: 15mins

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